The incorrect statement is:a)The second ionization energy of Se is greater than that of second ionization energy of Asb)The first ionizat ion energy of C2+ ion is greater than that of first ionizat ion energy of N2+ ion.c)The third ionizat ion energy of F is greater than that of third ionization energy of Od)Helogens have highest I.E. in respective periodCorrect answer is option 'D'. Can you explain this answer?

Question

Answer

Incorrect Statement: Helogens have the highest I.E. in respective periods.

Explanation:
Ionization energy (I.E.) is defined as the minimum amount of energy required to remove an electron from a neutral gaseous atom or ion. It is measured in electron volts (eV) or kilojoules per mole (kJ/mol). The ionization energy increases across a period due to the increase in the effective nuclear charge and decreases down a group due to the increase in the atomic size.

The given statement is incorrect because halogens do not always have the highest ionization energy in their respective periods. There are some exceptions to this trend due to the electronic configuration of some elements.

Exceptions to the trend of increasing I.E. across a period:
1. Group 3A elements (B, Al, Ga, In) have lower I.E. than Group 2A elements (Be, Mg, Ca, Sr, Ba) due to the presence of a stable half-filled p orbital in the former group.

2. Group 6A elements (O, S, Se) have higher I.E. than Group 5A elements (N, P, As) due to the presence of paired electrons in the p orbital of Group 6A elements.

3. Group 8A elements (He, Ne, Ar, Kr, Xe, Rn) have higher I.E. than Group 7A elements (F, Cl, Br, I, At) due to the stable electronic configuration of the former group.

4. Group 2B elements (Zn, Cd, Hg) have higher I.E. than Group 1B elements (Cu, Ag, Au) due to the fully filled d orbitals in the former group.

Exceptions to the trend of decreasing I.E. down a group:
1. There is a small increase in I.E. from Group 2A to Group 3A due to the smaller size of Group 3A elements and the shielding effect of d electrons.

2. There is a small increase in I.E. from Group 5A to Group 6A due to the increased effective nuclear charge and the presence of paired electrons in the p orbitals of Group 6A elements.

Conclusion:
In conclusion, the statement that halogens have the highest I.E. in their respective periods is incorrect. There are exceptions to this trend due to the electronic configuration of some elements. Therefore, it is important to consider the electronic configuration and other factors when predicting the ionization energy of an element.

Answer

Here in option d it is given that halogen have highest I.E but according to the trend in periodic properties noble gases have highest I E.

Answer

Because Nobel gases have the highes IE in the respective period.

Answer

Halogen gains one elctron to complete its octet configuration.so it's elctron gain enthalpy ( electron affinity) is high.

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